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States of Matter

States of Matter. Chapter 13. Kinetic Theory . Kinetic energy is energy due to motion. According to the kinetic theory, all matter consist of particles in constant motion. Three Assumptions of the Kinetic Theory.

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States of Matter

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  1. States of Matter Chapter 13

  2. Kinetic Theory Kinetic energy is energy due to motion. According to the kinetic theory, all matter consist of particles in constant motion

  3. Three Assumptions of the Kinetic Theory • The particles in a gas are considered to be hard small spheres with insignificant volume • No attractive or repulsive forces exist • Independent motion • Rapid, constant, random motion • Gases fill their containers • They travel in straight-line paths • The collisions are perfectly elastic • Energy Transferred without loss • Total energy remains the same

  4. Gas Pressure Results from the force exerted by a gas per unit of surface area Gas pressure is the result of simultaneous collisions of rapidly moving particles If no particles, then no collisions, so no pressure

  5. Gas Pressure Atmospheric Pressure results from collisions of atoms in the air with objects Decreases as elevation increases. Ex. Climbing a mountain A barometer measure atmospheric pressure

  6. Units for Pressure SI unit is Pascal (Pa) (this in now a base unit) Standard Units 1 atm = 760 mm Hg = 101.3 kPa = 760 torr = 1 N/m2 = 14.7 psi Have to convert between these units of pressure

  7. Conversions A pressure gauge records 460 kPa. What is the pressure in mmHg? Practice Time!

  8. Kinetic Energy and Temperature Potential Energy = stored energy As temperature increases, kinetic energy increases As a substance cools, kinetic energy decreases

  9. Kelvin SI unit The Kelvin temperature scale reflects the relationship between temperature and average kinetic energy Based on absolute zero of O K – the point at which all motion ceases

  10. States of Matter Solid Liquid Definite volume Definite shape Particles close together Vibrate Definite Volume No definite shape Particles further apart than solid Flow

  11. State of Matter Gas Plasma No definite volume or shape Far apart as possible Gas-like substance Very high temperatures Above 5000C Charged particle Ex. The sun

  12. Changes in States of Matter (Phase Changes) Melting Freezing Solid to liquid Increase in Kinetic energy Liquid to Solid Decrease in kinetic energy

  13. Changes in State Sublimation Deposition Solid directly to a gas Kinetic Energy Increases Ex. Iodine, dry ice, moth balls Gas directly to a solid Kinetic Energy Decreases

  14. Changes in State Vaporization Condensation Liquid to Gas KE increases Gas to Liquid KE decreases

  15. Review Kinetic Energy Increases solid liquid gas Kinetic Energy Decreases Gas liquid Solid

  16. Two Types of Vaporization • Evaporation – changes liquid to gases below boiling point • Cooling process • Boiling Point – when heated to a temperature in which particles have enough Kinetic Energy to vaporize

  17. Terms Normal Boiling Point – the boiling temperature of a substance at standard pressure Vapor Pressure – measure of the force exerted by a gas above a liquid

  18. Phase Diagrams Shows the relationship among solid, liquid, and vapor of a substance Gives the conditions (temperature and pressure) at which a substance exist as a solid, liquid or vapor

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